JEE Main 202622 JanuaryMorning Shift
- Exam
- JEE Main
- Year
- 2026
- Date
- 22 January
- Shift
- Morning Shift
- Subject
- Chemistry
- Chapter
- Haloalkanes and Haloarenes
JEE Main 2026 · 22 January · Morning Shift · Chemistry · Haloalkanes and Haloarenes
As compared with chlorocyclohexane, which of the following...
As compared with chlorocyclohexane, which of the following statements correctly apply to chlorobenzene?
A. The magnitude of negative charge is more on chlorine atom.
B. The bond has partial double bond character.
C. bond is less polar.
D. bond is longer due to repulsion between delocalised electrons of the aromatic ring and lone pairs of electrons of chlorine.
E. The bond is formed using hybridised orbital of carbon.
Choose the correct answer from the options given below:
A. The magnitude of negative charge is more on chlorine atom.
B. The bond has partial double bond character.
C. bond is less polar.
D. bond is longer due to repulsion between delocalised electrons of the aromatic ring and lone pairs of electrons of chlorine.
E. The bond is formed using hybridised orbital of carbon.
Choose the correct answer from the options given below:
Options
- AB, C and E Only
- BA, C and E Only
- CA, D and E Only
- DB, C and D Only
Correct answer
A. B, C and E Only
Step-by-step solution
Chlorobenzene has Cl attached to an sp² carbon of the benzene ring, while chlorocyclohexane has Cl attached to an sp³ carbon.
Statement B is correct: the C-Cl bond has partial double bond character due to resonance with the aromatic π system, where chlorine's lone pairs interact with the aromatic ring.
Statement C is correct: the C-Cl bond is less polar in chlorobenzene because the resonance contribution reduces the electronegativity difference between C and Cl.
Statement E is correct: the C-Cl bond is formed using sp² hybridized orbital of carbon.
Statement A is incorrect because chlorine carries less negative charge due to resonance donation to the aromatic system.
Statement D is incorrect because the C-Cl bond is actually shorter in chlorobenzene due to partial double bond character, not longer.
The correct statements are B, C, and E only.
Statement B is correct: the C-Cl bond has partial double bond character due to resonance with the aromatic π system, where chlorine's lone pairs interact with the aromatic ring.
Statement C is correct: the C-Cl bond is less polar in chlorobenzene because the resonance contribution reduces the electronegativity difference between C and Cl.
Statement E is correct: the C-Cl bond is formed using sp² hybridized orbital of carbon.
Statement A is incorrect because chlorine carries less negative charge due to resonance donation to the aromatic system.
Statement D is incorrect because the C-Cl bond is actually shorter in chlorobenzene due to partial double bond character, not longer.
The correct statements are B, C, and E only.